Ion-Ion interactions > Hydrogen bonds > Dipole-dipole interactions > Dispersion forces.
Hydrogen bonds are weaker in comparison to ion-ion interactions. This is due to the fact that hydrogen bonds are produced due to electronegativity and the bonding pair of the electron does not get inside the atom shell. On the other hand, the transfer of electrons occurs in ionic bonds, that is, the exchange of electrons occurs in ion-ion interactions.
Dipole-dipole interactions are weaker in comparison to hydrogen bonds. The dipole-dipole interactions prevail when partial negative charge arises on one polar molecule and a partial positive charge on another one. This attraction is only because of the existence of opposite charges on the polar molecule. These are, therefore, weaker interactions in comparison to hydrogen bonds.
Dispersion forces are weaker in comparison to dipole-dipole interactions. The dispersion forces are the weakest forces as they are temporary attractive forces. It is a result of the formation of temporary dipoles. Thus, these are weaker in comparison to dipole-dipole interactions.
Weakest : dispersion forces, dipole-dipole interactions, hydrogen bonding, ion-ion interactions : Strongest.
Negative is it can't be broken down and makes the air polluted. Positive, it can be re used again and again.
a) 18.81% is the mass percent (m/m) of the KCl solution.
b) 3.643 M is the molarity of the KCl solution.
c) 0.6073 M is the molarity of the diluted KCl solution.
a) mass on of evaporating dish = 24.10 g = x
mass on of evaporating dish and KCl solution = 44.30 g = y
After heating, mass on of evaporating dish and dry KCl = 27.90 g = z
Mass of KCl solution = y - x = 44.30 g - 24.10 g = 20.2 g
Mass of KCl in solution = z - x = 27.90 g - 24.10 g = 3.8 g
The mass percent (m/m) of the KCl solution;
18.81% is the mass percent (m/m) of the KCl solution.
b) Moles of KCl =
Volume of the KCl solution = 14.0 mL = 0.014 L ( 1 mL = 0.001 L)
Molarity of the solution :
3.643 M is the molarity of the KCl solution.
Molarity of KCl solution before dilution =
Volume of the solution before dilution =
Molarity of KCl solution after dilution =
Volume of the solution after dilution =
0.6073 M is the molarity of the diluted KCl solution.